JEE Questions for Chemistry Classification Of Elements And Periodicity In Properties Quiz 7 - MCQExams.com

On descending a group, valence electrons remain the same

Among the isoelectronic species, the size increases as the negative charge increases

Molecules F₂, Cl₂ and anion F^- (due to inert gas Ne configuration ) have almost zero electron affinity

Argon (3s² 3p⁶ ) has almost zero electron affinity

Both As and Bi belongs to group 15 of the periodic table and therefore, posses five electrons in the outermost orbit.

Na⁺ (11-1) and Ne (10) are isoelectronic

All these species are isoelctronic (14 electrons) and contain B.O. three

IE₁ decreases from top to bottom in a group

Size of an anion is larger than the corresponding atom and the ionization energy generally increases as the size decreases with increasing atomic number in a period.

Ionization energy decreases on moving top to bottom in a group

Rb, K Li and Cs are the alkali metals corresponding to the atomic numbers given

Element with At. No. 56 has the electronic configuration [Xe] 6 s² and thus belongs to s-block of the periodic table.

IE₁ of Li < Be > B < C or IE₁ of Li < B < Be < C.

Be has fully filled 2s-subshell (2s²) and therefore, shows least tendency to accept an electron. Thus, Be^‒ is least stable

According to periodic law of elements, the variation in properties of elements is related to their atomic numbers (electronic config.)

Electropositive character decreases form left to right across a period

Like covalent radii, van der Waals’ radii also decrease along a period from left to right due to increasing nuclear charge. Now N, O, F and Ne belong to the same (2^nd) period. Therefore, their van der Waals’ radii will increase in the order: Ne, F, O, N, Further, since Cl lies in third period, its van der Waals’ radius would be largest. Thus the overall increasing sequence is: Ne, F, O, N, Cl

Une stands for unnilennium which is the German name for 109

Rb (2.11 Å) is much larger than O(0.73 Å). since the size of cation is smaller while that of the anion is larger than the parent atom, therefore, the sizes of RB⁺( 1.48 Å) and O^2- (1.45 Å) coincidently match each other.

The sizes of Li⁺(0.68 Å) and Mg²⁺ (0.65 Å) being diagonally related are nearly the same.The sizes of Fe(1.17 Å) and Co(1.16 Å) are nearly the same because the contractive effect of the increased nuclear charge is counter balanced by increase in size due to increased shielding effect of the inner electrons

The size of K will be higher than that of K⁺ while size of F will be lower than that of F^-

The exceptional outer electronic configuration of Pd suggests that, in principle its configuration should have been 4d⁸ 5s². As such it lies in 5^th period and group 10.

None. Review the definitions of ionization enthalpy, electron gain enthalpy and electronegativity

First ionization enthalpies of Si, P, S and Cl are 786, 1012, 999, 1256 kJ mol^-1 respectively.Now follow the order of the elements and write their values accordingly

Due to stability of the [Rn] core, the filling of 5f orbitals does not begin until there are two electrons in the 6d-orbital and similarly, due to stability of the [Xe] core, the filling of 4f-orbitals does not occur until there is one electron in the 5 d-orbital. As such, the only true d-block element is (d).

In the isoelectronic series all isoelectronic anions belongs to the same period and cations to the next period.

The m.p./b.p. of the elements of group 17 increases down the group while those of groups 1.2 and 13 decrease down the group

Three complete subshells ( 1s² 2s² 2p⁶).